Question

which of these graphs best represents the relationship between the volume and temperature of a gas when the pressure and number of moles of the gas are kept constant?

Explanation:

Step1: Recall Charles's Law

Charles's Law states that \( V \propto T \) (when \( P \) and \( n \) are constant), which can be written as \( V = kT \) (\( k \) is a constant). This is a linear relationship with a zero - intercept.

Step2: Analyze the graphs

• The first graph (a curve) does not represent a linear \( V - T \) relationship.
• The second graph (a straight line passing through the origin) represents \( V = kT \) (since when \( T = 0\), \( V=0\) according to Charles's Law).
• The third graph (a horizontal line) implies \( V \) is constant with respect to \( T \), which is not in line with Charles's Law.

Answer:

The second graph (the straight - line graph passing through the origin) best represents the relationship.